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Investigating the rate of reaction between Hydrochloric acid and magnesium

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Introduction

Investigating the rate of reaction between Hydrochloric acid and magnesium Planning I am investigating the rate of reaction between HCl and Mg. I will change the concentration of my acid and see how this effects the rate of reaction. In this experiment I predict that the higher the concentration of the acid the quicker the rate of reaction will occur. This is because if the concentration is high there will be more acid molecules in a smaller space this means more collusions will take place resulting in the rate of reaction increasing. As magnesium is a group two metal it is quite reactive as it reacts with water. When a metal (Mg) reacts with an acid (HCl) it forms a salt (MgCl) and hydrogen. So here is the equation for this experiment: Mg + 2HCl = MgCl + H A reaction occurs when molecules collide with each other. However they need a certain amount of force to be able to react this is called activation energy. In my experiment I am investigating with different concentrations of acid . I predicted that the higher the concentration the quicker the reaction would take place. ...read more.

Middle

different ways firstly I will time how long it takes for a 1cm long strip of magnesium to disappear in the above concentrations. Secondly I will time how long it takes for 5cm of magnesium ribbon to produce 30cm of hydrogen. I will do each experiment twice so I will have more reliable data. Therefore I will have 4 results for each concentration, which should show clear trends. Method I carried out my first experiment by getting 25ml of acid I then put this into a beaker. Next I collected 1cm of magnesium ribbon and a stop clock. I dropped the magnesium in and timed how long it took for the magnesium to disappear. I then did the same for each of the other concentrations. For the second experiment I gathered a side armed flask, a bung, a piece of rubber tubing, and a gas syringe. I fitted these together by attaching the tubing to the side armed flask and the gas syringe. I then collected by acid and 5cm of magnesium, I then put both the acid and magnesium into the side armed flask and put the bung on tightly so no gas leaked out. ...read more.

Conclusion

was in the lower concentration of acid, this means there will be more successful collisions resulting in the rate of reaction going up. Most of my results support my prediction and even the two slightly odd results still show the same general pattern. Evaluation I think this was a successful experiment as my results show clear trends, which I have supported with scientific backup. My prediction was correct and I think I have sufficient deference to support my findings and decision, as I did 4 tests for each concentration. I think my results are reliable however, with improved equipment we could have made this experiment more precise, as some gas may have leaked out of the tubing. If I was to do this experiment again I would use equipment that would be more accurate at measuring the volume of gas produced. However I would probably still use concentration as my variable, because is easy to measure out concentrations and they gave be quite accurate results. To extend this activity I could do tests with more concentrations to backup my findings even more. I could also get other people to do the experiment as I may do the experiment in a different way to others, so this would give me a better overall average. ...read more.

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